Ions and Ionic Compounds l OBJECTIVES: –Determine the number of valence electrons in an atom of a representative element.

Ions and Ionic Compounds l OBJECTIVES: –Explain octet rule

Ions and Ionic Compounds l OBJECTIVES: –Describe how cations form.

Ions and Ionic Compounds l OBJECTIVES: –Explain how anions form.

Valence Electrons are… l responsible for chemical properties l Valence electrons - The s and p electrons in the outer energy level

Keeping Track of Electrons l Atoms in the same column... –same outer electron configuration. –same valence electrons. l Number of valence electrons = the group number for a representative element

Electron Dot diagrams are… l A way keeping track of valence electrons. l Write the symbol - it represents the nucleus and inner (core) electrons l Put one dot for each valence electron (8 maximum) l They don’t pair up until they have to (Hund’s rule) X

The Electron Dot diagram for Nitrogen l Nitrogen has 5 valence electrons l First we write the symbol. N l Then add 1 electron at a time to each side. l Now they are forced to pair up. l We have now written the electron dot diagram for Nitrogen.

The Octet Rule l Noble gases are unreactive in chemical reactions l 1916, Gilbert Lewis explain why atoms form certain kinds of ions and molecules l The Octet Rule: atoms tend to achieve noble gas configuration l Each noble gas (except He) has 8 electrons in the outer level

Formation of Cations l Metals lose electrons to attain a noble gas configuration. l Make positive ions (cations) l Na 1s 2 2s 2 2p 6 3s 1 1 valence electron l Na 1+ 1s 2 2s 2 2p 6 This is a noble gas configuration with 8 electrons in the outer level.

Electron Dots For Cations l Metals have few valence electrons (usually 3 or less); calcium has only 2 valence electrons Ca

Electron Dots For Cations l Metals have few valence electrons l Metals will lose the valence electrons Ca

Electron Dots For Cations l Metals have few valence electrons l Metals will lose the valence electrons l Forming positive ions Ca 2+ NO DOTS are now shown for the cation. This is named the calcium ion.

Electron Configurations: Anions l Nonmetals gain electrons to attain noble gas configuration. l Make negative ions (anions) l S = 1s 2 2s 2 2p 6 3s 2 3p 4 = 6 valence electrons l S 2- = 1s 2 2s 2 2p 6 3s 2 3p 6 = noble gas configuration.

Electron Dots For Anions l Nonmetals will have many valence electrons (usually 5 or more) l They will gain electrons to fill outer shell. P P 3- This is called the phosphide ion

Stable Electron Configurations l All atoms react to try and achieve a noble gas configuration. l Noble gases have 2 s and 6 p electrons. l 8 valence electrons = already stable! l This is the octet rule (8 in the outer level is particularly stable). Ar

Ionic Compounds l OBJECTIVES: –Explain the electrical charge of an ionic compound.

Ionic Compounds l OBJECTIVES: –Describe three properties of ionic compounds.

Ionic Bonding l Anions and cations held together by opposite charges. l Ionic compounds = salts. l Simplest ratio = formula unit. l Held together by transfer of electrons. l Electrons are transferred to achieve noble gas configuration.

Ionic Bonding NaCl The metal (sodium) tends to lose its one electron from the outer level. The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.

Ionic Bonding Na + Cl - Note: Remember that NO DOTS are now shown for the cation!

Ionic Bonding l All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable). CaP Lets do an example by combining calcium and phosphorus:

Ionic Bonding CaP

Ionic Bonding Ca 2+ P

Ionic Bonding Ca 2+ P Ca

Ionic Bonding Ca 2+ P 3- Ca

Ionic Bonding Ca 2+ P 3- Ca P

Ionic Bonding Ca 2+ P 3- Ca 2+ P

Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

Ionic Bonding Ca 2+ P 3- Ca 2+ P 3- Ca 2+

Ionic Bonding = Ca 3 P 2 Formula Unit This is a chemical formula, which shows the kinds and numbers of atoms in the smallest representative particle of the substance. For an ionic compound, the smallest representative particle is called a: Formula Unit

Properties of Ionic Compounds l Crystalline solids - repeating arrangement of ions in the solid: Fig. 7.9, page 197 l Ions are strongly bonded together. –Structure is rigid. –High melting points l Coordination number- number of ions of opposite charge surrounding it

Do they Conduct? l Conducting electricity means allowing charges to move. l In a solid, the ions are locked in place. l Ionic solids are insulators. l When melted, the ions can move around. l Melted ionic compounds conduct. –NaCl: must get to about 800 ºC. l Dissolved in water, they also conduct (free to move in aqueous solutions)

- Page 198 The ions are free to move when they are molten (or in aqueous solution), and thus they are able to conduct the electric current.

Metals and Metalic Bonding l OBJECTIVES: –Model the valence electrons of metal atoms.

Metals and Metalic Bonding l OBJECTIVES: –Describe the arrangement of atoms in a metal.

Metals and Metalic Bonding l OBJECTIVES: –Explain the importance of alloys.

Metallic Bonds are… l How metal atoms are held together in the solid. l Metals hold on to their valence electrons very weakly. l Think of them as positive ions (cations) floating in a sea of electrons:

Sea of Electrons l Electrons are free to move through the solid. l Metals conduct electricity.

Metals are Malleable l Hammered into shape (bend). l Also ductile - drawn into wires. l Both malleability and ductility explained in terms of the mobility of the valence electrons

- Page 201 1) Ductility2) Malleability Due to the mobility of the valence electrons, metals have: and Notice that the ionic crystal breaks due to ion repulsion!

Malleable Force

Malleable l Mobile electrons allow atoms to slide by, sort of like ball bearings in oil. Force

Ionic solids are brittle Force

Ionic solids are brittle l Strong Repulsion breaks a crystal apart, due to similar ions being next to each other. Force

Crystalline structure of metal l If made of one kind of atom, metals are among the simplest crystals; very compact & orderly l Note Fig. 7.14, p.202 for types: 1. Body-centered cubic: –every atom (except those on the surface) has 8 neighbors –Na, K, Fe, Cr, W

Crystalline structure of metal 2. Face-centered cubic: –every atom has 12 neighbors –Cu, Ag, Au, Al, Pb 3. Hexagonal close-packed –every atom also has 12 neighbors –different pattern due to hexagonal –Mg, Zn, Cd

Alloys l We use lots of metals every day, but few are pure metals l Alloys are mixtures of 2 or more elements, at least 1 is a metal l made by melting a mixture of the ingredients, then cooling l Brass: an alloy of Cu and Zn l Bronze: Cu and Sn

Why use alloys? l Properties are often superior to the pure element l Sterling silver (92.5% Ag, 7.5% Cu) is harder and more durable than pure Ag, but still soft enough to make jewelry and tableware l Steels are very important alloys –corrosion resistant, ductility, hardness, toughness, cost

Why use alloys? l Types? a) substitutional alloy- the atoms in the components are about the same size l b) interstitial alloy- the atomic sizes quite different; smaller atoms fit into the spaces between larger l “Amalgam”- dental use, contains Hg